Question

An empty 5.00-l flask is charged with 0.300 g of pure h2s(g), at 25 ∘c.

Answer 1

The student's question is related to calculating the total pressure in a mixture of gases using Dalton's Law of Partial Pressures and the ideal gas equation, P = (nRT)/V, where R is the universal gas constant.

Step-by-step explanation:

The question asked by the student involves calculating the total pressure in a flask containing multiple gases at a given temperature using the ideal gas law. This is a classic chemistry problem involving gas laws, specifically Dalton's Law of Partial Pressures, which states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of individual gases. To compute the total pressure, one would use the formula P₁ = (n₁RT)/V, where n₁ is the number of moles of gas, R is the universal gas constant, T is the temperature in Kelvin, and V is the volume of the flask. The pressure for each gas is calculated and then added together to find the total pressure.

Answer 2

To evaluate the statements relating to the formation of H2S, we determine whether each statement is true or false. Then, we calculate the initial pressure of H2S in the flask using the ideal gas law.

To evaluate the statements, we need to consider the reaction for the formation of H2S from its elements: H2(g) + S(g) ⇌ H2S(g).

a) False - A reaction does occur as H2S is formed.

b) False - The pressure of ammonia is not relevant to the question.

c) True - Q is greater than K when the reaction is not at equilibrium.

d) False - The reaction proceeds to the right (forward) side to form H2S.

e) False - Q is not equal to zero since the reaction occurs.

f) True - The reaction proceeds to the right side.

To find the initial pressure of H2S, we convert the given mass of H2S to moles using its molar mass.

0.350 g / (34.08 g/mol) = 0.0102 mol.

The initial pressure can be determined using the ideal gas law:

PV = nRT

P = (nRT) / V

P = (0.0102 mol * 0.0821 atm/mol*K * 298 K) / 5.00 L

P = 0.00485 atm

The complete question is here:

An empty 5.00-L flask is charged with 0.350g of pure H2S(g), at 25 ?C.

Part A

Evaluate the validity of the following statements.

TRUE OR FALSE

a) no reaction occurs.

b) the pressure of ammonia is zero.

c) Q is greater than K

d) the reaction proceeds to the left.

e)Q is equal to 0.

f) the reaction proceed to the right.

Part B

What is the initial pressure of H2S(g) in the flask?

Express your answer numerically in atmospheres