A 50.0 mL sample of a gas was found to have a pressure of 1.0 atm at 25 degree C

Question

A 50.0 mL sample of a gas was found to have a pressure of 1.0 atm at 25 degree C. What will be the new volume if the pressure is changed to 0.50 at constant temperature? The temperature of 20.0 mL of certain gas was changed from 25.0 degree C to 50 degree C at constant pressure. What is the new volume of the gas in mL? Calculate: (i) The number of atoms in 2.50 g of potassium (ii) The number of molecules in 3.00 g of nitrogen gas, N_2 A 1.00 L sample of chlorine gas at 25.0 degree C was found to have a pressure of 1.00 atm. How many moles of gas are present and what is the mass of the gas in grams? Calculate the volume of CO_2 gas at STP obtained by reacting a 10.00 g sample of calcium carbonate with an excess of hydrochloric acid: CaCO_3 (s) + 2 HCl (aq) rightarrow CaCl_2 (aq) + CO_2 (g) + H_2 O (l) A student prepared Na_2 CO_3 by bubbling CO_2 through an aqueous solution of NaOH: 2 NaOH (aq) + CO_2 rightarrow Na_2 CO_3 (aq) + H_2 O (l) If 15.0 g of NaOH was used, what mass of Na_2 CO_3 is expected?

Explanation / Answer

Question 1.

V = 50 mL of a gas

P = 1 atm

T = 25°C = 298 K

find ne wvolume if P = 0.5 atm at T constant

Apply ideal gas law ratios

P1*V1 = P2*V2

1*50 = 0.5*V2

V2 = 50/0.5 = 100 mL

the new volume is expected to double, i.e. 100 mL

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