The pressure, p, of a gas varies directly with its temperature, t, and inversely with its volume, v, according to the equation p=nrt/v, where n is the number of molar units and r is the universal gas constant. one molar unit of gas has a pressure of about 1,245 joules at a temperature of 300 degrees kelvin and a volume of 2 liters. what is the pressure of the same number of molar units of the gas at a temperature of 400 degrees kelvin and a volume of 2.5 liters?

The pressure of gas will be 1328 Joules

Step-by-step explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

  (for same value of n)

where,

= initial pressure of gas = 1245 J

= final pressure of gas = ?

= initial volume of gas = 2 L

= final volume of gas = 2.5L

= initial temperature of gas = 300K

= final temperature of gas = 400K

Now put all the given values in the above equation, we get the final pressure of gas.

Therefore, the final pressure of gas will be 1328 Joules.

the mistake in the pattern is that :

b. the decimal point was moved one too many place values each time

the correct pattern could be made by :

b. moving the decimal point to the right the same numbers of place values as the exponents

14.3

step-by-step explanation:

add all the numbers together.

9 + 12 + 15 + 16 + 17 + 17 = 86

now, divide 86 by how many numbers we have: 6.

86 / 6 = 14.3