Answer:
Explanation:
Repeated tests help determine whether the hypothesis is always true in different circumstances. Repeatedly testing a hypothesis qualifies it to be accepted as a theory.
Water is the component that is produced here.
Main Answer:
Given data:
Initial Pressure P1 = 570 mm hg
Initial Volume V1 = 2270 ml
Final Pressure P2 = ? mm hg
Final Volume V1 = 1250 ml
According to the ideal gas equation,
PV = constant.
P1V1 = P2V2
P2 = P1V1/V2
P2 = (570 x 2270) / 1250
P2 = 1035.12 mm hg
The final pressure at volume of 1250 ml is 1035.12 mm hg.
Explanation:
What is ideal gas equation ?
The ideal gas equation is as follows:
PV = nRT
where P = Pressure
V = Volume
n = number of moles of gas
R = Universal gas constant
T = Temperature
This ideal gas equation provides the macroscopic particles behavior of the gas. At this condition, the particles of the gas, won't be attract or repel each other. It is consider as the stable condition.
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What we can actually do is to find the number of moles of Ca.
moles Ca = 0.72 g / (40.08 g/mol) = 0.018 mol
From the given choices, we can all see that there are 1 mol of compound
per 1 mole of Ca. Therefore the actual moles of compound is also 0.018 mol.
From this, calculate the mass and the answer is the one which will give 2 g.
Answer:
D. CaCl2
Answer:
The empirical formula is C2H5O
Explanation:
Step 1: Data given
Suppose the mass of the compound = 100.0 grams
The compound contains:
53.31 % C = 53.31 grams C
11.18 % H = 11.18 grams H
35.51 % O = 35.51 grams O
Step 2: Calculate moles
moles = mass / molar mass
Moles C = 53.31 grams / 12.01 g/mol
Moles C = 4.439 moles
Moles H = 11.18 grams / 1.01 g/mol
Moles H = 11.07 moles
Moles O = 35.51 grams / 16.0 g/mol
Moles O = 2.22 moles
Step 3: Calculate mol ratio
We divide by the smallest amount of moles
C: 4.439 / 2.22 = 2
H: 11.07 / 2.22 = 5
O: 2.22/2.22 = 1
C2H5O
The empirical formula is C2H5O
