Here are mass spectrometric signals for methane in H2:

CH2 (Vol %) 0 0.062 0.122 0.245 0.486 0.971 1.921

Signal (mV) 9.1 47.5 95.6 193.8 387.5 812.5 1671.9

a) Subtract blank value from all other values. Then use the method of least squares to find the slope and intercept and their uncertainties.

b)Replicate measurements of an unknown gave 152.1, 154.9, 153.9, and 155.1 mV and a blank gave 8.2, 9.4, 10.6, and 7.8 mV. Subtract average blank from average unknown to find average corrected signal for the unknown.

c) Find concentration of the unknown and uncertainty.

Expert Solution

Colby Messinger answered 2 years ago

Methane is synthesized with a stoichiometric mixture of CO and H2 that is produced via a...

Methane is synthesized with a stoichiometric mixture of CO and H2 that is produced via a large scale coal gasification process CO + 3H2 = CH4 + H2O over Ni/Alumina catalyst. (a) What is the equilbrium conversion you can get at 400oC and 1 atm? (b) Because of exothermic nature of the reaction, reaction temperature inside a large scale commercial reactor could be raised to 700oC even if the feed temperature is kept at 350oC. Estimate the equilibrium conversion at...

A 1:3 mixture of CO and H2 is passed through a catalyst to produce methane at...

A 1:3 mixture of CO and H2 is passed through a catalyst to produce methane at 500 K. CO(g) + 3H2(g) = CH4(g) + H2O(g) How much heat is liberated in producing a mole of methane? How does this compare with the heat obtained from burning a mole of methane at this temperature? How does the heat of combustion of CH4 compare with the heat of compustion of CO+3H2? (Answers: 206.11 kJ is liberated; Burning CH4 liberates 802.34 kJ; Burning...

2. Based on the mass of methane that was combusted, how much energy was released in...

2. Based on the mass of methane that was combusted, how much energy was released in GJ? Assume the energy content for natural gas is 55 MJ/kg. 6.4117 x 1011 kg of methane is combusted = 6.4117 x 1011 x 55 MJ = 352.6435 x 1011 MJ 352.6435 x 1011 MJ = 352.6435 x 1011 x 0.001 GJ = 352.6435 x 108 GJ of energy was released. 3. Based on the mass of methane that was combusted, what mass of...

Calculate the mass of methane that must be burned to provide enough heat to convert 266.0...

Calculate the mass of methane that must be burned to provide enough heat to convert 266.0 g of water at 39.0°C into steam at 110.0°C. (Assume that the H2O produced in the combustion reaction is steam rather than liquid water.)

Calculate the mass of methane that must be burned to provide enough heat to convert 300.0...

Calculate the mass of methane that must be burned to provide enough heat to convert 300.0 g of water at 30.0°C into steam at 106.0°C.

Calculate the mass of methane that must be burned to provide enough heat to convert 347.0...

Calculate the mass of methane that must be burned to provide enough heat to convert 347.0 g of water at 18.0°C into steam at 110.0°C. (Assume that the H2O produced in the combustion reaction is steam rather than liquid water.)

Twenty kg of a fuel consisting of 50% methane, 25% ethane and 25% propane (by mass)...

Twenty kg of a fuel consisting of 50% methane, 25% ethane and 25% propane (by mass) is compressed to 180 atm and 100 degrees C. What is the compressed volume using Kay’s rule?

The formula for methane is CH4 and it’s molar mass is 16.04 grams/mol. (a) How many...

The formula for methane is CH4 and it’s molar mass is 16.04 grams/mol. (a) How many moles of methane are in 2.750 grams of methane? (b) How many molecules of methane are in a 11.5 mole sample?

Methane (CH4) enters a compressor operating at steady state with a mass flow rate of 170...

Methane (CH4) enters a compressor operating at steady state with a mass flow rate of 170 lbm/hr. The methane enters the compressor at p1 = 15 lbf/in2 , T1 = 80F and exits at p2 = 100 lbf/in2 . The work input to the compressor is 15 hp. Assume ideal gas behavior for the methane with constant specific heats (cp = 0.538 Btu/lbm·R, cv = 0.414 Btu/lbm·R). Kinetic and potential energy effects are negligible and the compressor is insulated 1)Determine...

Determine the mass (in grams) of magnesium metal required to produce 40.0 mL of H2 with...

Determine the mass (in grams) of magnesium metal required to produce 40.0 mL of H2 with a temperature of 26.9 oC and an atmospheric pressure of 745 mmHg. Be sure to take into account water vapour. 3. A sample of a halogen gas has a mass of 0.538 g and exerts a pressure of 600.0 torr at 14.0 oC in a 100.0 mL flask. Calculate the molar mass of the halogen gas. Is the halogen gas F2, Cl2, Br2 or...

Question