What is the approximate temperature of 1.4 moles of a gas with a pressure of 3.25 atmospheres in a 4.738-liter container

134K

Explanation:

Using the ideal gas law equation;

PV = nRT

Where;

P = pressure (atm)

V = volume (Litres)

n = number of moles (mol)

R = gas constant (0.0821 Latm/Kmol)

T = temperature (K)

Based on the information provided, n = 1.4moles, P = 3.25atm, V = 4.738L, T = ?

3.25 × 4.738 = 1.4 × 0.0821 × T

15.3985 = 0.11494T

T = 15.3985/0.11494

T = 133.969

Approximately;

T = 134K

i think it is d. e because the next one is igneous.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: