IMOLK Data, Trial 2 Ideal Gas Law-PV=nRT Molarity of HCI (M): Data, Trial 1 3.00M 3.00 M Volume of HCI (ml): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 22.5°C Temperature (°C): 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt: Mg + 2 HCl 1MgCl₂ + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water. (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R=

IMOLK Data, Trial 2 Ideal Gas Law-PV=nRT Molarity of HCI (M): Data, Trial 1 3.00M 3.00 M Volume of HCI (ml): 20 ml 20 mL Mass of Mg (g): 03429 .03309 Volume of gas (ml): 42.5mL 45.0ml Barometric Pressure (mm Hg): 760 760 22.5°C Temperature (°C): 22.5°C Write the balanced molecular equation for the reaction of magnesium and HCI to form hydrogen gas and the magnesium salt: Mg + 2 HCl 1MgCl₂ + H₂ Mole of Mg reacted Mole of H₂ formed (based on the Balanced equation for the reaction) Vapor Pressure of water. (from curve in mmHg): Pressure of H₂ from Dalton's Law (in mmHg) Pressure of H₂ in atm Volume of H₂ in liter Temperature in Kelvin Calculation of R Percent error Average R=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

I need solutions for all parts
asap please
What is the mole fraction of O2 in a mixture that is 115 g N2 and 88.0 g O2? mole/mole What am I doing incorrect? O2- 32g/mol; N2-28 g/mol O: 88/32=2.75mol O N: 115/28=4.107mol N 2.75+4.107=6.857 2.75 (O2mol)/6.9 (total mol)= 0.3985 O2 mols I entered: 0.399 for 3 SF it was incorrect, I got 3 SF from the # of Grams Then entered: 0.40 also incorrect...
I just need help on number 2 because I am confused
How many Liters (O2) are consumed, STP, if 59.9grams C2H6 is burned C2H6(g) + O2 -> CO2(g) + H2O(g) (please balance) 2C2H6+5O2 -> 2CO2 + 6H2O (???)
If the density of HNO₃ is 1.5 g/L and its 0.945M , what the ( %v/w ) of HNO₃ H= 1 , N = 14 , O = 16
Dd.10.
Please provide only typed answer solution no handwritten solution needed allowed
Please use complete format
Need help asap
Question 2 of 10 -/3 View Policies Current Attempt in Progress A bubble of air escaping from a diver's mask rises from a depth of 197 ft to the surface where the pressure is 1.00 atm. Initially, the bubble has a volume of 10.0 mL. Assuming none of the air dissolves in the vwater, how mnany times larger is the bubble just as it reaches the surface? Use this data: 1. The density of seawater is approximately 1.025 g mL1 2. The density of mercury is 13.6 g mL1 times larger Use your answer to explain why scuba divers constantly exhale as they slowly rise from a deep dive. Since the pressure v by a factor of approximately i , the volume must v by a factor of approximately Divers exhale to the amount of gas in their lungs, so it does not v to a volume vthan the diver's lungs. !!
5-What volume of hydrogen gas at STP is produced from the reaction of 31.49 g of Mg? Balance the equation: ____Mg + ____ HCl -> ____MgCl2 + ____H2