Environmentally conscious Susan has been toldthat a new electric car will only generate 6 ounces of green-house gases (GHG) per mile, but that a standard internalcombustion car is double that at 12 ounces per mile. However,the nature of electric cars is such that the new technology andelectric batteries generate 30,000 lbs. of GHG to manufactureand another 10,000 lbs. to recycle. A standard car generatesonly 14,000 lbs. of GHG to manufacture, and recycling withestablished technology is only 1,000 lbs. Susan is interested intaking a systems approach that considers the life-cycle impactof her decision. How many miles must she drive the electriccar for it to be the preferable decision in terms of reducinggreenhouse gases?

Please help, will provide helpful ratings for correct solution. (Gpt/Ai wrong ans not allowed) Q.A reaction at 18.0 °C evolves 603. mmol of sulfur tetrafluoride gas. Calculate the volume of sulfur tetrafluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Be sure your answer has the co number of significant digits. volume: L x10 X

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

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7. When detern ing the mass of a liquid, ras in a hurry and did not allow enough time for the temperature of the flask to reach the temperature of the boiling water bath. The student recorded the temperature of the gas as 100.0°C when it was only 80.0°C, Is the molar mass calculated by the student higher or lower than the accepted molar mass, or does this error have no effect on the calculated result? Briefly explain your answer # 2/HB Office DEPOTS b) If the student assumed the volume of the flask was 125 mL (as marked by the side of the flask) rather than measuring the volume experimentally, would the unknown's calculated molar mass be too high, too low, or unaffected? Explain. # 2/HB 4

A 335 mL sample of oxygen gas at 25 °C is heated to 50 °C. What is the final volume of the gas (in mL)? (Assume constant P) (Show Work)