A7.70 l 7.70 l container holds a mixture of two gases at 47 ° c. 47 °c. the partial pressures of gas a and gas b, respectively, are 0.344 atm 0.344 atm and 0.893 atm. 0.893 atm. if 0.190 mol 0.190 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

1.884 atm

Explanation:

We have at first, a mix of two gases A and B, with a pressure and temperature. The total pressure of this mix is the sum of both pressures fo these gases so:

P = 0.344 + 0.893 = 1.237 atm

Now after this, a third gas is added but there is no change in temperature or volume, which means that this gas may have a behavior of ideal gas, therefore, we can use the expression for ideal gas which is:

P = nRT/V

R is the gas constant, in this case is 0.082 L atm/ K mol

Replacing all the values that we have of volume and temperature, we can calculate the pressure that this gas exert:

P = 0.19 * 0.082 * (47+273.15) / 7.7

P = 0.647 atm

Now the total pressure, we add this value and we have:

P' = 1.237 + 0.647

P' = 1.884 atm

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.

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