$(P_1V_1)/T_1=(P_2V_2)/T_2$, given a constant quantity of gas. And thus, $(P_1xxV_1xxT_2)/(V_2xxT_1)=P_2$, even given this format, we can see the problem is dimensionally sound. We do need to use $"absolute temperature."$ $P_2=(1.00*atmxx250*mLxx313*K)/(500*mLxx293*K)~=1/2*atm.$
1 Answers 1 viewsThis is an example of Gay Lussac's temperature-pressure gas law , which states that the pressure of a gas held at constant volume, is directly proportional to the temperature in...
1 Answers 1 viewsstates that the volume of an enclosed gas is inversely proportional tot he pressure exerted on it, provided the temperature remains constant. $therefore P_1V_1=P_2V_2$ $therefore V_2=(P_1V_1)/P_2$ $=(236xx60)/354$ $=40m^3$
1 Answers 1 views...according to the combined gas equation... We solve for....$V_2=(P_1V_1)/T_1xxT_2/P_2$ $=(150*kPaxx200*L)/(273*K)xx(546*K)/(600*kPa)=??*L$
1 Answers 1 viewsUse the : $P_1 V_1 = P_2 V_2$ . substituting and making the units consistent: $(200xx10^3)(2500)=(500xx10^3)(V_2)$. solve for $V_2$ .
1 Answers 1 viewsConcept of is to be applied here. Let the partial pressure of $Ar$ in the final mixture be $p_"Ar"$ Initially before mixing $ Ar$ had Pressure $P_"Ar"=1.29$ atm Temperature$T_"Ar"=223+273=500$...
1 Answers 1 viewsHere's how I go about doing this. What we can do is use the ideal gas equation for both $"Ar"$ and $"O"_2$ to find the total moles. Then we...
1 Answers 1 views$P*V=n*R*T " " $(Ideal gas law) Assuming that the amount of gas and the temperature are fixed, the product of the pressure and volume is constant at any given moment....
1 Answers 1 viewsThis is an example of the . The equation to use is $(P_1V_1)/(T_1)=(P_2V_2)/(T_2)$. Given Initial pressure, $P_1="250 kPa"$ Initial volume, $V_1="15 m"^3"$ Initial temperature, $T_1="100 K"$ Final pressure, $P_2="500 kPa"$...
1 Answers 1 viewsEven without doing any calculations, you should be able to look at the information given and predict that the volume of the gas will increase after temperature is increased and...
1 Answers 1 views