Answer:
FeCl2 + H. 2
Explanation:
Iron react with hydrogen chloride to produce iron(II) chloride and hydrogen.
A) Aerobic Respiration.
Respiration<span> releases energy for cells from </span>glucose<span>.</span> Aerobic respiration, needs oxygen, while anaerobic does not. Oxygen is produced alongside glucose in photosynthesis, not used. Fermentation occurs in anaerobic conditions (without oxygen).
The average atomic mass of chromium to 3 decimal points is 52. 055 g. mol.
<h3>What is the average atomic mass?</h3>
"The weighted average mass of the atoms in a naturally occurring sample of an element is the average atomic mass, also known as atomic weight."
Given the different isotopes of chromium.
The four isotopes of chromium are cr-50, cr-52, cr-53 cr-54.
The average atomic mass will be
Let us take the weighted average of your isotopes:
50 × 0.0434 + 52 × 0.8379 + 53 × 0.095 + 54 × 0.0237 = 52. 055 g.
Thus, the average atomic mass of chromium is 52. 055 g.
To learn more about average atomic mass, refer to the link:
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<span>pre-1982 definition STP: 120 g/mol
post-1982 definition STP: 122 g/mol
The answer to this question depends upon which definition of STP you're using. The definition changed in 1982 from 273.15 K at 1 atmosphere to 273.15 K at 10000 pascals. As a result the molar volume of a gas at STP changed from 22.4 L/mol to 22.7 L/mol. So let's calculate the answer using both definitions and see if your text book is 35 years obsolete.
First, determine the number of moles of gas you have. Do this by dividing the volume you have by the molar volume. So
pre-1982: 0.04665 / 22.4 = 0.002082589 mol
post-1982: 0.04665 / 22.7 = 0.002055066 mol
Now divide the mass you have by the number of moles.
pre-1982: 0.250 g / 0.002082589 mol = 120.0428725 g/mol
post-1982: 0.250 g / 0.002055066 mol = 121.6505895 g/mol
Finally, round to 3 significant figures:
pre-1982: 120 g/mol
post-1982: 122 g/mol
These figures are insanely large for nitrogen gas. So let's see if our input data is reasonable. Looking up the density of nitrogen gas at STP, I get a value of 1.251 grams per liter. The value of 0.250 grams in the problem would then imply a volume of about one fifth of a liter, or about 200 mL. That is over 4 times the volume given of 46.65 mL. So the verbiage in the question mentioning "nitrogen gas" is inaccurate at best.
I see several possibilities.
1. The word "nitrogen" was pulled out of thin air and should be replaced with "an unknown"
2. The measurements given are incorrect and should be corrected.
In any case, if #1 above is the correct reason, then you need to pick the answer based upon which definition of STP your textbook is using.</span>
