Can somebody explain this ideal gas law problem?

Question

I need help understanding the ideal gas law in general.

calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas.

A. What volume of carbon dioxide gas is produced from this amount of calcium carbonate. The gas is measured at .95atm and 10 degrees celcius.

Answer 1

ok from what i understand the ideal gas law is this:

PV = NRT (pressure x volume = number of moles x the constant x temperature) am i right?

in this case, the pressure is 0.95 (convert this to kilopascals)

R i think = 8.314? (not sure of this value)

temperature is 10 degrees = 283 kelvin

substitute these values into the equation

sori im in a rush here hope this helps in some way

Answer 2

CaCO3   --->  CaO + CO2

    PV = nRt

      V =  nRt / p

      

......... sorry but i'm stuck here .... :(

Do you have the mass of the gas? or number of mole of the gas?