Acylinder, with a piston pressing down with a constant pressure, is filled with 1.90moles of a gas (n1), and its volume is 48.0l (v1). if 0.800mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?

and

a sample of gas in a cylinder as in the example in part a has an initial volume of 70.0l , and you have determined that it contains 2.00moles of gas. the next day you notice that some of the gas has leaked out. the pressure and temperature remain the same, but the volume has changed to 17.5l . how many moles of gas (n2) remain in the cylinder?

Part A: 27.8 L; Part B: 0.500 mol

Explanation:

Part A

For an ideal gas, we can use the equation:

PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

In the beggining:

P*48.0 = 1.90*RT

P/RT = 1.90/48.0

P/RT = 0.03958

For constants pressure and temperature, after 0.800 mol of gas leaks out: n = 1.90 - 0.800 = 1.10 mol

PV = 1.10*R*T

P/RT = 1.10/V

0.03958 = 1.10/V

V = 1.10/0.03958

V = 27.8 L

Part B

In the beginning

PV = nRT

P*70.0 = 2.00*RT

P/RT = 2.00/70.0

P/RT = 0.02857

After the gas leaked out:

PV = nRT

P*17.5 = nRT

P/RT = n/17.5

0.02857 = n/17.5

n = 0.500 mol

your answer is c

hope i ! ; )

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.