The ideal gas law states that for a gas confined to a container with volume V at temperature T, the pressure P exerted on the container wall is given by P = RT/V, where R is an empirically determined constant. (In this equation, volume is measured in cubic centimeters and temperature in Kelvin.) Suppose that an ideal gas is in a vessel with volume 1000 cm3 at 600 K. Which will have a bigger effect on pressure, a small decrease in volume or a small increase in temperature?
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