Question 2 3 pts
In the reaction 2C2H6 + 702 --> 4CO2 + 6H20
If 955.291 grams of oxygen are used how many grams of water will be made? (Put down only the
number of grams with the correct number of significant figures but no units. The significant figures
will be limited by the periodic table. Make sure to use the Periodic table from the course.)

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

the answer is 303.15 or 303

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

is there any options? maybe im just not seeing them but i need the options to

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