Two identical cylinders, a and b, contain the same type of gas at the same pressure. cylinder a has twice as much gas as cylinder b. which is true? a. ta = tbb. not enough information to make a comparison. c. ta > tbd. ta < tb

D. TA < TB

Explanation:

From general gas equation, we know that:

PV  = nRT

PV/R = nT

where,

P = pressure of gas

V = volume of gas

R = General gas constant

T = temperature of gas

n = no. of moles of gas

FOR CYLINDER A:

PV/R = (nA)(TA)   eqn (1)

FOR CYLINDER B:

PV/R = (nB)(TB)   eqn (2)

Because, Pressure, Volume are constant for both cylinders.

Comparing eqn (1) and (2)

(nA)(TA) = (nB)(TB)

It is given that the amount of gas in cylinder A is twice as much as the gas in cylinder B. This means the number moles in cylinder A are twice as much as no. of moles in cylinder B.

nA = 2(nB)

using this in eqn:

2(nB)(TA) = (nB)(TB)

TA = (1/2)(TB)

TA = 0.5 TB

Therefore it is clear that the correct option is:

D. TA<TB

answer; ///i believe that the correct answer is (carbon); good luck

vapour or gas assuming atmospheriv pressure