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Mrac [35]
3 years ago
8

Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC2(s) + 2H2O(l)C2H2(g) + Ca(OH

)2(aq) The product gas, C2H2, is collected over water at a temperature of 25 °C and a pressure of 759 mm Hg. If the wet C2H2 gas formed occupies a volume of 8.19 L, the number of moles of CaC2 reacted was ______ mol. The vapor pressure of water is 23.8 mm Hg at 25 °C.
Chemistry
1 answer:
poizon [28]3 years ago
7 0

Answer:

33.7

Explanation:

i just know i had a question on it'

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ASAP please
choli [55]
D.
0.220/0.2= 1.10 M
5 0
2 years ago
If you had 6 moles of CaCl2 and 5 moles of Na3PO4, which of these would be the limiting and excess reactant
faltersainse [42]

Answer:

Na3PO4 is excess reactant, CaCl2 is limiting reactant.

Explanation:

                                      3CaCl2 + 2Na3PO4 ---> Ca3(PO4)2 + 6NaCl

from reaction :              3 mol        2 mol

given:                            6 mol         5 mol (X)

X = (6*2)/3 = 4 mol Na3PO4

For 6 mol CaCl2 we need 4 mol Na3PO4, but  we have 5 mol Na3PO4,

Na3PO4 is excess reactant, so CaCl2 is limiting reactant.

8 0
3 years ago
Calculate the oxidation number of the iodine (I) in each compound: HIO4 = I2 = NaI = HIO3 =
Makovka662 [10]
1) in periodic acid (HIO₄), iodine has oxidation number +7, hydrogen has oxidation number +1, oxygen has -2, compound has neutral charge:
+1 + x + 4 · (-2) = 0.
x = +7.

2) in molecule of iodine (I₂), iodine has oxidation number 0, because iodine is nonpolar molecule.

3) in sodium iodide (NaI), iodine has oxidation number -1, sodium has oxidation number +1:
+1 + x = 0.
x = -1.

4) in iodic acid (HIO₃), iodine has oxidation number +5, hydrogen has oxidation number +1, oxygen has -2, compound has neutral charge:
+1 + x + 3 · (-2) = 0.
x = +5.
8 0
3 years ago
Read 2 more answers
Another chemistry question i’m not good at this at all:( has me stressed
adoni [48]

Answer:

Average atomic mass = 15.86 amu.

Explanation:

Given data:

Number of atoms of Z-16.000 amu = 205

Number of atoms of Z-14.000 amu = 15

Average atomic mass  = ?

Solution:

Total number of atoms = 205 + 15 = 220

Percentage of Z-16.000 = 205/220 ×100 = 93.18%

Percentage of Z-14.000 = 15/220 ×100 = 6.82 %

Average atomic mass  = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass)  / 100

Average atomic mass  = (93.18×16.000)+(6.82×14.000) /100

Average atomic mass =  1490.88 + 95.48 / 100

Average atomic mass =  1586.36 / 100

Average atomic mass = 15.86 amu.

5 0
3 years ago
According to the equation below, how many moles of PbO are required to generate 3.88×1023 nitrogen molecules?
saul85 [17]

Answer:

1.935 mole

Explanation:

We'll begin by calculating the number of mole present in 3.88x10^23 molecules of nitrogen(N2). This can be obtained as follow:

From Avogadro's hypothesis, 1 mole of any substance contains 6.02x10^23 molecules. Therefore 1 mole of N2 contains 6.02x10^23 molecules.

Now if 1 mole of N2 contains 6.02x10^23 molecules,

Then Xmol of N2 will contain 3.88x10^23 molecules i.e

Xmol of N2 = (3.88x10^23)/6.02x10^23

Xmol of N2 = 0.645 mole

Now, we can obtain the number of moles of PbO required to generate 3.88x10^23 molecules (i.e 0.645 mole) of N2. This is illustrated below:

The equation for the reaction is given below:

3PbO + 2NH3 → 3Pb + N2 + 3H2O

From the balanced equation above, 3 moles of PbO produced 1 mole of N2.

Therefore, Xmol of PbO will produce 0.645 mole of N2 i.e

Xmol of PbO = 3 x 0.645

Xmol of PbO = 1.935 mole.

From the calculations made above,

1.935 mole of PbO will produce 3.88x10^23 molecules of nitrogen (N2).

8 0
3 years ago
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