A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 1200. mL at a pressure of 1.00 atm, and it weighs 1.27 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

A sample of an unknown compound is vaporized at  100.°C . The gas produced has a volume of  1330.mL  at a pressure of  1.00atm , and it weighs  4.52g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits.

A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 1850. mL at a pressure of 1.00 atm, and it weighs 1.95 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits. g mol x10 X

A sample of methane occupied 18.95 L at 41.03 °C. When the volume changed to 11.60 L at 16.59 °C, the pressure was 2.044 atm. Calculate the original pressure (atm). Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 =  V1 =  T1= n1= P2= V2= T2= n2=   Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2…