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For many purposes we can treat nitrogen (N) as an ideal gas at temperatures above its boiling point of -196. C. Suppose the temperature of a sample of nitrogen gas is raised from -13.0°C to 24.0°C, and at the same time the pressure is changed. If the initial pressure was 7.0 atm and the volume decreased by 35.0%, what is the final pressure? Round your answer to the correct number of significant digits.

Answers

Answer 1

Answer:

Answer: 22.8atm

Explanation:

T1 = —13°C = —13 +273 = 260K

T2 = 24°C = 24 +273 = 297K

V1 = V

V2 = 35% of V= 0.35V

P1 = 7atm

P2 =?

P1V1/T1 = P2V2 /T2

(7 x V)/260 = (P2 x 0.35V)/297

P2x0.35Vx260 = 7V x 297

P2 x 91V = 2079V

P2 = 2079V / 91V

P2 = 22.8atm

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Consider the following reaction at equilibrium. What effect will adding 1.4 mole of He to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g) Consider the following reaction at equilibrium. What effect will adding 1.4 mole of He to the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g) The reaction will shift to the left in the direction of reactants. No effect will be observed. The reaction will shift to the right in the direction of products. The equilibrium constant will increase. The equilibrium constant will decrease.

Answers

Answer:

The reaction will shift to the left in the direction of reactants.

Explanation:

According to Le Chatelier's principle, when an external constraint is applied to a chemical system in equilibrium, the system adjust in order to annul the effect impose on it by the external system.

Also, from the principle, the addition of an inert gas can affect the equilbrium of a gaseous system, but only if the volume is allowed to change.

There are two cases on which equilibrium depends. These are:

1. Addition of an inert gas at constant volume:

When an inert gas is added to the system in equilibrium at constant volume, the total pressure will increase. But the concentrations of the products and reactants (i.e. ratio of their moles to the volume of the container) will not change. Hence, there will be no effect on the equilibrium.

2. Addition of an inert gas at constant pressure:

When an inert gas is added to a system in equilibrium at constant pressure, then the total volume will increase(i.e. the number of moles per unit volume of various reactants and products will decrease). Hence, the equilibrium will shift towards the direction in which there is increase in number of moles of gases.

Considering the given reaction in equilibrium:

2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

The addition of an inert gas at constant pressure to the above reaction will shift the equilibrium towards the backward direction because the number of moles of reactants is more than the number of moles of the products.

Final answer:

Adding 1.4 moles of He to the reaction mixture will have no effect on the equilibrium of the system.

Explanation:

Adding 1.4 moles of He to the reaction mixture will have no effect on the system. The equilibrium of the reaction will not shift to the left or right, and there will be no change in the equilibrium constant. This is because He is considered an inert gas and does not participate in the reaction.

Learn more about Effect of adding He to a reaction mixture here:

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Glucose, C 6 H 12 O 6 , is used as an energy source by the human body. The overall reaction in the body is described by the equation C 6 H 12 O 6 ( aq ) + 6 O 2 ( g ) ⟶ 6 CO 2 ( g ) + 6 H 2 O ( l ) Calculate the number of grams of oxygen required to convert 58.0 g of glucose to CO 2 and H 2 O . mass of O 2 : 61.76 g Calculate the number of grams of CO 2 produced.

Answers

Answer:

$m_(O_2)=61.87gO_2$

$m_(CO_2)=85.07gCO_2$

Explanation:

Hello,

Considering the given reaction's stoichiometry, grams of oxygen result:

$m_(O_2)=58.0gC_6H_(12)O_6*(1molC_6H_(12)O_6)/(180gC_6H_(12)O_6)*(6molO_2)/(1molC_6H_(12)O_6)*(32gO_2)/(1molO_2)\nm_(O_2)=61.87gO_2$

Moreover, the mass of produced carbon dioxide turns out:

$m_(CO_2)=58.0gC_6H_(12)O_6*(1molC_6H_(12)O_6)/(180gC_6H_(12)O_6)*(6molCO_2)/(1molC_6H_(12)O_6)*(44gCO_2)/(1molCO_2)\nm_(O_2)=85.07gCO_2$

Best regards.

Combustion of Solid Fuel. A fuel analyzes 74.0 wt % C and 12.0% ash (inert). Air is added to burn the fuel, producing a flue gas of 12.4% CO2, 1.2% CO, 5.7% O2, and 80.7% N2. Calculate the kg of fuel used for 100 kg mol of outlet flue gas and the kg mol of air used. (Hint: First calculate the mol O2 added in the air, using the fact that the N2 in the flue gas equals the N2 added in the air. Then make a carbon balance to obtain the total moles of C added.)

Answers

Answer:

Kg of fuel used = 220.54Kg

Explanation:

The concept of material balance is applied here by taking into consideration the percentage composition of each flue gas in the atmosphere. This is used with each of the percentage composition of the flue gas that burn in the fuel and the detailed steps is as shown in the attachment.

Water flows over Niagara Falss at the average rate of 2,400,000 kg/s, and the average height of the falls is about 50 m. Knowing that the graviatational potential energy of falling water per second = mass (kg) x height (m) x gravity (9.8 m/s2), what is the power of Niagara Falls? How many 15 W LED light bulbs could it power?

Answers

Answer:

1. 176 × 10^12 W ; 78400000000

Explanation:

Given the following :

Fall rate = 2,400,000kg/s

Average height of fall = 50m

Gravitational Potential of falling water = mgh = mass × acceleration due to gravity × height =

How many 15 W LED light bulbs could it power?

Recall : power = workdone / time

Workdone = gravitational potential energy

Mass of water = density * volume

Density of water = 1 * 10^3kg/m^3

Rate of fow = volume / time = 2400000

Hence,

Power = 1000 * 2,400,000 * 9.8 * 50

Power = 1176000000000

Power = 1. 176 × 10^12 W

How many 15 W LED light bulbs could it power?

1176000000000 / 15 = 78400000000

= 78400000000 15 W bulbs

After clamping a barrette to a ring stand you noticed that the set up is tippy and unstable what should you do to stabilize the set up?

Answers

Move the buret clamp to a ring stand with a larger base.

Which best illustrates the way in which radiation transfers thermal energy?

#edge2021

Answers

Answer:

it's b.

Explanation:

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First one
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