Agas sample has an initial pressure of 547 mmhg and an initial volume of 0.500 l. what is the pressure (in atm) if you decrease the volume of the sample to 225 ml?

To solve this, we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 =P2V2

P2 = P1 x V1 / V2

P2 = 547 mmHg x 500 mL / 225 mL

P2 =1215.56 mmHg

1215.56 mmHg ( 1 atm / 760 mmHg) = 1.60 atm

Therefore, the new pressure of the gas would be 1.60 atm.

the answer is true. hope it .

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol