A patient has been diagnosed with mitochondrial disease and is experiencing the following symptoms: fatigue (lack of energy)and muscle weakness. Which organelles (cell parts) would NOT likely be immediately responsible for these symptoms? select all that apply. Mitochondria,Chloroplast, Lysosome,and Cytoplasm.NEED HELP ASAP

Answers

Answer 1

Answer:

Answer:

Chloroplast, Lysosome

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During an experiment, a student adds 2.90 g CaO to 400.0 mL of 1.500 M HCl . The student observes a temperature increase of 6.00 °C . Assuming that the solution's final volume is 400.0 mL , the density is 1.00 g/mL , and the heat capacity is 4.184 J/g⋅°C , calculate the heat of the reaction, ΔHrxn .

Answers

Answer:

ΔHrxn = 193107.69 J/mol

Explanation:

ΔHrxn = mcΔT

m = mass

c = heat capacity

ΔT = temperature variation

density = m/V

m = density x V

m = 1.00 g/mL x 400.0 mL

m = 400.0 g

ΔHrxn = mcΔT

ΔHrxn = 400 g x 4.184 J/g°C x 6.00 °C

ΔHrxn = 10041.6 J

CaO + 2HCl → CaCl₂ + H₂O

CaO = 56.0774 g/mol

2.90 g CaO = 0.052 mol

400.0 mL of 1.500 mol/L HCl = 0.6 mol HCl

ΔHrxn = 10041.6 J is for 0.052 mol of CaO

ΔHrxn = 193107.69 J is for 1 mol of CaO

Using a density of 1.0 g/mL for the water added and adding in the mass of the lithium nitrate, what is the total mass of the solution?

Answers

The total mass of the solution of lithiumnitrate solution has been 99.7 grams.

Density can be defined as the mass of the solute per unit volume. The density can be expressed as g/ml or kg/L.

The mass of given Lithium nitrate = 2.5 grams.

The mass of water can be given as:

Density = $\rm (Mass)/(Volume)$

Volume of water = 97.2 ml.

The total mass of solution:

Mass of water = Density $*$ Volume

Mass of water = 1 $*$ 97.2 grams

Mass of water = 97.2 grams

The total mass = Mass of lithium nitrate + mass of water

= 2.5 + 97.2 grams

= 99.7 grams.

The total mass of the solution of lithiumnitrate solution has been 99.7 grams.

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Answer:

The total mass of the solution = 99.7 g

Note: The question is incomplete. The complete question is given below:

A "coffee-cup" calorimetry experiment is run for the dissolution of 2.5 g of lithium nitrate placed into 97.2 mL of water. The temperature of the solution is initially at 23.5oC. After the reaction takes place, the temperature of the solution is 28.3 oC.

1. Using a density of 1.0 g/mL for the water added and adding in the mass of the lithium nitrate, what is the total mass of the solution and solid?

Explanation:

mass = density * volume

density of water = 1.0 g/mL; volume of water = 97.2 mL

mass of water = 1.0 g/L * 97.2 mL

mass of water = 97.2 g

mass of lithium nitrate = 2.5 g

A solution is made by dissolving a solute (usually solid) in a solvent (usually a liquid). The solute in this reaction is lithium nitrate and the solvent is water.

Total mass of solution = mass of water + mass of lithium nitrate

Total mass of solution = 97.2 g + 2.5 g = 99.7 g

Therefore, total mass of the solution = 99.7 g

A sample of nitrogen occupies a volume of 500ml at 60 and 500 mm hg of pressure. what will its volume be at stp\

Answers

Answer : The volume at STP will be 0.2944 L

Solution : Given,

Initial volume = 500 ml

Initial temperature = $60^oC=273+60=333K$ $(0^oC=273K)$

Initial pressure = 500 mmHg = $(500)/(760)=.658atm$ $(1atm=760mmHg)$

At STP,

Temperature = 298 K

Pressure = 1 atm

Formula used : $(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$

where,

$P_1$ = initial pressure

$P_2$ = pressure at STP

$T_1$ = initial temperature

$T_2$ = temperature at STP

$V_1$ = initial volume

$V_2$ = volume at STP

Now put all the given values in this formula, we get

$((0.658atm)* (500ml))/(333K)=((1atm)* V_2)/(298K)$

By rearranging the terms, we get the volume at STP

$V_2=294.42ml=0.2944L$ (1 L = 1000 ml)

Therefore, the volume at STP will be 0.2944 L

Final answer:

To find the volume of nitrogen at STP, we need to use the ideal gas law equation.

Explanation:

To find the volume of nitrogen at STP, we need to use the ideal gas law equation. The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the universal gas constant, and T is temperature in Kelvin. At STP, the pressure is 1 atm and the temperature is 273 K. Plug in the given values and solve for V:

V = (500 mL * 500 mmHg * (1 atm / 760 mmHg))/(0.0821 L·atm/mol·K * 333 K)

V = 162.6 mL

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Cobalt chloride Select one: a. Forms a single hydrate which may be pink or blue
b. Is colorless in the presence of water
c. Does not exist as a hydrate
d. Forms different hydrates which have different colors

Answers

Answer:Forms different hydrates which have different colors

Explanation:

CoCl2 in its anhydrous form is blue in colour. This anhydrous compound could absorb moisture, first forming the purple dihydrate and absorbs more water molecules to form the hexahydrate. Hence various hydrates of cobalt II chloride have different colours as stated above. Equations of reaction for the formation of the two hydrates are attached.

A piece of charcoal used for cooking is found at the remains of an ancient campsite. a 0.94 kg sample of carbon from the wood has an activity of 1580 decays per minute. find the age of the charcoal. living material has an activity of 15 decays/minute per gram of carbon present and the half-life of 14c is 5730 y. answer

Answers

Mass of sample of charcoal = 0.94 kg = 0.00094

∴, activity = decay rate / mass = 1580/0.00094
= 1.681 X 10^6 decays per min per gram

Using the half-life formula, we have:
activity of sample / activity of modern carbon = (1/2)^(age / half-life)
∴, Age = half-life x log (base 2) (modern activity / coal activity)
= 5730 x log(base 2)(1.681X10^6/ 15)
= 96115 years.

Answer: Age of the charcoal = 96115 years

Final answer:

Using the radiocarbon dating technique and applying the decay formula, it is calculated that the age of the charcoal from the an ancient campsite is approximately 9,500 years.

Explanation:

The age of the charcoal can be found using the technique of radiocarbon dating, which capitalizes on the process of radioactive decay. The isotope carbon-14 (¹4C) is used in this method as it has a known half-life of 5730 years. The number of decays per minute per gram of carbon in a live organism is known as its activity.

Initially, the activity was given as 15 decays per minute per gram. The present activity of the carbon in the charcoal is provided at 1580 decays per minute for a 0.94 kg or 940 gram sample. Thus, the current activity per gram is 1580/940 equals approximately 1.68 decays per minute per gram.

Given that the half-life of ¹4C is 5730 years, we can apply the formula for calculating the time passed using the rate of decay, which is given as T = (t1/2 / ln(2)) * ln(N0/N), where 'ln' is the natural logarithm, 'N0' is the initial quantity (15 decays/minute per gram), 'N' is the remaining quantity (1.68 decays/minute per gram).

Plugging in the given values, we get T = (5730 / ln(2)) * ln(15/1.68), which gives us approximately 9,500 years. Therefore, the age of the charcoal is around 9,500 years.

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Use the equation editor or "Insert Chemistry - WIRIS editor" to write the balanced molecular chemical equation for the reaction of aqueous 0.13 M lead (II) nitrate, with 0.19 M potassium carbonate. You may need to consult Appendix E to determine the states of each reactant and product. Assume any insoluble products are completely insoluble.