If 3.21 mol of a gas occupies 56.2L at 44C and a pressure of 793 torr, what volume will 5.29 mol of this gas occupy under the same conditions?

(A) 61.7 L
(B) 30.9 L
(C) 14.7 L
(D) 92.6 L
(E) 478 L

is it d, 92.6 L?

Looks ok to me.

Great, thank you!

To solve this problem, we can use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, let's convert the given temperature from Celsius to Kelvin:

T = 44°C + 273.15 = 317.15 K

Now let's rearrange the ideal gas law equation to solve for V:

V = (n × R × T) / P

Substituting the given values into the equation:

V₁ = (3.21 mol × R × 317.15 K) / 793 torr

Since we are considering the same conditions, we can assume that R is a constant, so we can simplify the equation:

V₁ = (3.21 mol × constant) / 793 torr

Now, we need to find the constant value. The value of R depends on the units we use for pressure and volume. In this case, the units of pressure are torr, and the units of volume are liters. The value of R for this case is 0.0821 L·atm/(mol·K).

Plugging in the value of R into the equation:

V₁ = (3.21 mol × 0.0821 L·atm/(mol·K) × 317.15 K) / 793 torr

V₁ ≈ 0.325 L

Now, we can use the calculated value of V₁ to find the volume V₂ for 5.29 mol of the gas:

V₂ = (5.29 mol × 0.0821 L·atm/(mol·K) × 317.15 K) / 793 torr

V₂ ≈ 0.714 L

Now, since the answer choices are given in liters, we need to convert the volumes from liters to the correct number of significant figures provided.

The answer choice that is closest to 0.714 (rounded to the nearest tenth) is (C) 14.7 L.

Therefore, the correct answer is (C) 14.7 L, not (D) 92.6 L.