Which element is present in all organiccompounds?
(1) nitrogen
(2) oxygen
(3) carbon
(4) sulfur
Answers
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b) a period of time when temperatures across the planet are colder than normal
c) a characteristic of summer that returns seasonally
d) the gain of heat in coastal areas from El Niño storms
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Global Warming is a gradual increase in the overall temperature of the earth's atmosphere.
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a
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(2) 2H2O(l) + energy → 2H2(g) + O2(g)
(3) H2O(l) → H2O(s) + energy
(4) H2O(g) → H2O(l) + energy
Answers
The answer is B because energy was added to 2H2O in order to produce a chemical change of 2H2 and 02 seperately.
Final answer:
The balanced equation that represents a chemical change is 2H2O(l) + energy → 2H2(g) + O2(g).
Explanation:
The balanced equation that represents a chemical change is (2) 2H2O(l) + energy → 2H2(g) + O2(g). In this equation, we see the reactant, water (H2O), being converted into two separate products, hydrogen gas (H2) and oxygen gas (O2), with the addition of energy. This indicates a chemical change taking place where new substances are formed.
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Answer:
C15H24O
Explanation:
TO GET THE EMPIRICAL FORMULA, WE NEED TO KNOW THE MASSES AND CONSEQUENTLY THE NUMBER OF MOLES OF EACH OF THE INDIVIDUAL CONSTITUENT ELEMENTS.
FIRSTLY, WE CAN GET THE MASS OF THE CARBON FROM THAT OF THE CARBON IV OXIDE. WE NEED TO KNOW THE NUMBER OF MOLES OF CARBON IV OXIDE GIVEN OFF. THIS CAN BE CALCULATED BY DIVIVDING THE MASS BY THE MOLAR MASS OF CARBON IV OXIDE. THE MOLAR MASS OF CARBON IV OXIDE IS 44G/MOL
HENCE, THE NUMBER OF MOLES OF CARBON IV OXIDE IS 4.122/44 WHICH EQUALS 0.094. SINCE THERE IS ONLY ONE ATOM OF CARBON IN CO2 THEN THEY HAVE EQUAL NUMBER OF MOLES AND THUS THE NUMBER OF MOLES OF CARBON IS 0.094. WE CAN THEN PROCEED TO CALCULATE THE MASS OF CO2 PRESENT. THIS CAN BE CALCULATED BY MULTIPLYING THE NUMBER OF MOLES BY THE ATOMIC MASS UNIT. THE ATOMIC MASS UNIT OF CARBON IS 12. HENCE, THE MASS OF CO2 PRESENT IS 12 * 0.094 = 1.128g
WE CAN NOW GET THE MASS OF THE HYDROGEN BY MULTIPLYING THE NUMBER OF MOLES OF WATER BY 2 AND ALSO ITS ATOMIC MASS UNIT
TO GET THE NUMBER OF MOLES OF WATER, WE SIMPLY DIVIDE THE MASS BY THE MOLAR MASS. THE MOLAR MASS OF WATER IS 18g/mol. The NUMBER OF MOLES IS THUS 1.350/18 = 0.075
THE NUMBER OF MOLES OF HYDROGEN IS TWICE THAT OF WATER SINCE IT CONTAINS 2 ATOMS PER MOLECULE OF WATER. ITS NUMBER OF MOLES IS THUS 0.075*2 = 0.15 MOLE
THE MASS OF HYDROGEN IS THUS 0.075 * 2 * 1 = 0.15g
WE CAN NOW FIND THE MASS OF OXYGEN BY SUBTRACTING THE MASSES OF HYDROGEN AND CARBON FROM THE TOTAL MASS.
MASS OF OXYGEN = 1.376-0.15-1.128 = 0.098g
THE NUMBER OF MOLES OF OXYGEN IS THUS 0.098/16 = 0.006125
WE CAN NOW USE THE NUMBER OF MOLES TO OBTAIN THE EMPIRICAL FORMULA.
WE DO THIS BY DIVIDING EACH BY THE SMALLEST NUMBER OF MOLES WHICH IS THAT OF THE OXYGEN.
C = 0.094/0.006125 = 15
H = 0.15/0.006125 = 24
O = 1
THE EMPIRICAL FORMULA IS THUS C15H24O
The combustion of 1.376 g of butylated hydroxytoluene (BHT) produced 4.122 g CO2 and 1.350 g H2O. Calculations yield an empirical formula of CH2O, indicating one carbon, two hydrogen, and one oxygen atom.
To determine the empirical formula of butylated hydroxytoluene (BHT), we can follow these steps:
1. **Find moles of CO2 and H2O produced:**
\[ \text{moles of } CO_2 = \frac{\text{mass of } CO_2}{\text{molar mass of } CO_2} \]
\[ \text{moles of } H_2O = \frac{\text{mass of } H_2O}{\text{molar mass of } H_2O} \]
2. **Find the mole ratio:**
Divide the moles of each element (C, H, and O) in CO2 and H2O by the smallest number of moles.
3. **Write the empirical formula:**
Use the mole ratios to write the empirical formula.
Let's perform the calculations:
\[ \text{Molar mass of } CO_2 = 12.01 \, \text{(C)} + 2 \times 16.00 \, \text{(O)} = 44.01 \, \text{g/mol} \]
\[ \text{Molar mass of } H_2O = 2 \times 1.01 \, \text{(H)} + 16.00 \, \text{(O)} = 18.02 \, \text{g/mol} \]
\[ \text{moles of } CO_2 = \frac{4.122 \, \text{g}}{44.01 \, \text{g/mol}} \approx 0.0938 \, \text{mol} \]
\[ \text{moles of } H_2O = \frac{1.350 \, \text{g}}{18.02 \, \text{g/mol}} \approx 0.0749 \, \text{mol} \]
Divide by the smallest number of moles (0.0749) to get a ratio close to 1:1:
\[ \text{C} : \text{H} : \text{O} \approx 1.25 : 1 : 1 \]
The ratio is approximately 1:1:1, so the empirical formula is CH2O.
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Answer:
A) 2Na + = 2NaBr
Explanation:
As the problem says that you should find the balanced chemical equation for the synthesis of NaBr from Na and , the reactants are Na and
and the product is NaBr, so it can be writen as:
Na + = NaBr
Then you shoud balance the equation, it means that you should have the same number of each element in each part of the equation, so if you put a number 2 for the NaBr and the Na, the equation will be balanced:
2Na + = 2NaBr