If a gas has a volume of 1000 ml at a temperature of 23°c and a pressure of 100 mmhg, what is it’s volume under standard conditions of temperature and pressure?

119.7 mL.

Explanation:

From the general law of ideal gases:

PV = nRT.

where, P is the pressure of the gas.

V is the volume of the container.

n is the no. of moles of the gas.

R is the general gas constant.

T is the temperature of the gas (K).

For the same no. of moles of the gas at two different (P, V, and T):

P₁V₁/T₁ = P₂V₂/T₂.

P₁ = 100.0 mmHg, V₁ = 1000.0 mL, T₁ = 23°C + 273 = 296 K.P₂ = 1.0 atm = 760.0 mmHg (standard P), V₂ = ??? mL, T₂ = 0.0°C + 273 = 273.0 K (standard T).

∴ V₂ = (P₁V₁T₂)/(T₁P₂) = (100.0 mmHg)(1000.0 mL)(273.0 K)/(296 K)(760.0 mmHg) =  121.4 mL.

Sorry i dont understand the question can you rephase it?

Heat is involved in chemical change in two ways; chemical changes either result in heat being added to or removed from an object, and chemical changes require a certain amount of heat before they can take place.