EXERCISE 7 NAME LAB SECTION DATE Re Data Trial Mass of Mg (g) Initial volume of

Question

EXERCISE 7 NAME LAB SECTION DATE Re Data Trial Mass of Mg (g) Initial volume of Syringe (mL) Final volume of Syringe (mL) ayOnl &6.0ml 9Som/ Volume of H2 (mL) Barometric pressure (torr), Ambient temperature (C) 21 Vapor pressure of H2O (torr) deur 224 22.y ml 9m 21m 2a - Analysis Your goal is to determine the value of R from your data. Perform each of the following operations. Attach a page showing your work. You do not have to show work for every trial, but show your work for one sample trial for each step. 1. Determine the number of moles of magnesium consumed in the reaction, which will be equal to the number of moles of H2 produced (see Equation (2). Moles of Mg (g) Use Equation (2) to determine the pressure of H2 in the sample. Express your answer in 2 atmospheres. Pressure of H2 (atm) Convert the ambient temperature to Kelvin. Ambient temperature (K) Use Equation (1) to calculate R. Remember to convert mL to Lto get the units below. R (Latm/(mol K)) Calculate the average and standard deviation of your values of R. Average R (L atm/(mol K) Standard deviation in R (Latm/(mol K)

Explanation / Answer

Mole of Mg = mass/ molar mass

= 0.02/24

=0.00083 mole

Pressure of H2 =  

PV= nRT

P = nRT/V

= 0.00083* 0.083*297/0.024

= 0.8525 atm

K.= 24 c° +273

= 297 K

R = PV / nT

=0.85*0.024/ 0.00083*297

=0.070

Devaition= ,0.07/ 0.083*100

84.33%

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