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laila [671]
2 years ago
6

Which statement is true for a cooling curve​

Chemistry
1 answer:
rjkz [21]2 years ago
6 0

what are your choices

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What temperature in degrees c is the freezing point of water?
guajiro [1.7K]
The freezing point of water is 0° C. The Celsius (centigrade) scale is based off of water, with the freezing point at 0° and the boiling point at 100°. (Google will probably tell you this in 10 seconds, then you wouldn't have had to wait 7 hours!)
5 0
3 years ago
During the combustion of methane (CH4), one mole of methane gas combines with two moles of oxygen gas (O2) to produce one mole o
astraxan [27]

Answer:

CH4(g) +2O2____ CO2(g) +2H2O (l)

3 0
2 years ago
What volume would 312g of alcohol occupy
Aleksandr-060686 [28]

Answer:

Density=Mass/volume

0.91g/ml=312g/volume

Volume=343ml

Explanation:

3 0
3 years ago
3. A student carries out the clay-catalyzed dehydration of cyclohexanol starting with 10 moles of cyclohexanol and obtains 500 m
IrinaK [193]

Answer:

49.45~%

Explanation:

In this case, we have to start with the <u>chemical reaction</u>:

C_6H_1_2O~->~C_6H_1_0~+~H_2O

So, if we start with <u>10 mol of cyclohexanol</u> (C_6H_1_2O) we will obtain 10 mol of cyclohexanol (C_6H_1_0). So, we can calculate the grams of cyclohexanol if we<u> calculate the molar mass:</u>

(6*12)+(10*1)=82~g/mol

With this value we can calculate the grams:

10~mol~C_6H_1_0\frac{82~g~C_6H_1_0}{1~mol~C_6H_1_0}=820~g~C_6H_1_0

Now, we have as a product 500 mL of C_6H_1_0. If we use the <u>density value</u> (0.811 g/mL). We can calculate the grams of product:

500~mL\frac{0.811~g}{1~mL}=405.5~g

Finally, with these values we can calculate the <u>yield</u>:

%~=~\frac{405.5}{820}x100~=~49.45%%= (405.5/820)*100 = 49.45 %

See figure 1

I hope it helps!

6 0
3 years ago
if there are 4 grams of reactant,how many grams of product are produced by the chemical reaction. a.0 grams b.2 grams c.4 grams
Murrr4er [49]
4 grams , mass cannot be created or destroyed. it has to be the same on both sides of the equation
5 0
3 years ago
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