Response:1816.6 joules
Clarification:refer to the attached image
Every single-celled organism is able to survive because it carries out *
1 answer:
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Answer:
3.816 × 10⁻³ M
Explanation:
A stock solution of Cu²⁺(aq) is made by dissolving 0.8875 g of solid Cu(NO₃)₂∙2.5H₂O in a 100.0-mL volumetric flask, and then brought up to volume with water. What is the molarity (in M) of Cu²⁺(aq) in this stock solution?
We can derive the following relations:
- The molar mass of Cu(NO₃)₂∙2.5H₂O is 232.59 g/mol.
- Each mole of Cu(NO₃)₂∙2.5H₂O yields one mole of Cu²⁺.
The moles of Cu²⁺ present in 0.8875 g of Cu(NO₃)₂∙2.5H₂O are:
The molarity of Cu²⁺ is:
Response:
of
can be found in 39.5 grams of
.
Clarification:
Atomic weights: P= 31, F= 19,
The molar mass equals 1 atomic weight of P + 5 atomic weights of
F= 31+5 × 19 = 31+95
=126 g/mole
The number of moles in 39.5 gm of
equals
=
=0.3134 moles
1 mole of any substance encompasses
0.3131 moles comprises 0.3134
Thus, of
can be found in 39.5 grams of
.
Result: 1.68 L of liquid nitrogen is generated during the gas liquefaction process.
Clarification:
This process involves transforming gaseous nitrogen into its liquid form.
The two states possess distinct densities, thus occupying varying volumes; however, the mass remains constant.
Step 1: Calculate the mass of nitrogen gas
Let’s determine the mass of nitrogen gas associated with 297 L.
The density formula is:
With a density of nitrogen gas at 4.566 g/L and a volume of 297 L, we can compute the mass of nitrogen gas as follows:
Using these values yields:
The mass of nitrogen gas calculates to be 1356 g.
Step 2: Derive the volume of liquid nitrogen from the mass obtained
The mass for liquid nitrogen remains the same.
With the density of liquid nitrogen at 809 g/L, we can substitute this into our formula to find the volume of liquid.
Therefore, the volume of liquid nitrogen is 1.68 L.