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4 years ago

Would it be A or C???????? Helppp

Chemistry

2 answers:

stealth61 [152]4 years ago

8 0

Answer:

A. One that is not a fossil fuel

Explanation:

"Alternative fuel" is a technical term used in the fuel industry. It refers to fuels that that are not fossil fuels (like coal, oil, and natural gas).

B. is wrong. A fuel that hasn't been developed yet is not of much use.

C. is wrong. A homeowner may consider wood as an alternative fuel in case there is no electricity to power an oil furnace, but that is not the technical meaning of the term.

D. is wrong. An alternative fuel should use renewable resources.

Charra [1.4K]4 years ago

6 0

Answer:

Explanation:

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A solution of starch at room temperature does not readily decompose to form a solution of simple sugars because

Basile [38]

Explanation:

The starch requires a temperature higher than the room temperature (arround 60 °C) to decompose to form simple sugars. This is because the energy required to break the chemical bonds. Also, it may need the action of some specific enzymes (alpha and beta amilase) to break those bonds.

6 0

3 years ago

onsider the following reaction: CaCN2 + 3 H2O → CaCO3 + 2 NH3 105.0 g CaCN2 and 78.0 g H2O are reacted. Assuming 100% efficiency

mestny [16]

Answer : The excess reactant is, $H_2O$

The leftover amount of excess reagent is, 7.2 grams.

Solution : Given,

Mass of $CaCN_2$ = 105.0 g

Mass of $H_2O$ = 78.0 g

Molar mass of $CaCN_2$ = 80.11 g/mole

Molar mass of $H_2O$ = 18 g/mole

Molar mass of $CaCO_3$ = 100.09 g/mole

First we have to calculate the moles of $CaCN_2$ and $H_2O$ .

$\text{ Moles of }CaCN_2=\frac{\text{ Mass of }CaCN_2}{\text{ Molar mass of }CaCN_2}=\frac{105.0g}{80.11g/mole}=1.31moles$

$\text{ Moles of }H_2O=\frac{\text{ Mass of }H_2O}{\text{ Molar mass of }H_2O}=\frac{78.0g}{18g/mole}=4.33moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$CaCN_2+3H_2O\rightarrow CaCO_3+2NH_3$

From the balanced reaction we conclude that

As, 1 mole of $CaCN_2$ react with 3 mole of $H_2O$

So, 1.31 moles of $CaCN_2$ react with $1.31\times 3=3.93$ moles of $H_2O$

From this we conclude that, $H_2O$ is an excess reagent because the given moles are greater than the required moles and $CaCN_2$ is a limiting reagent and it limits the formation of product.

Left moles of excess reactant = 4.33 - 3.93 = 0.4 moles

Now we have to calculate the mass of excess reactant.

$\text{ Mass of excess reactant}=\text{ Moles of excess reactant}\times \text{ Molar mass of excess reactant}(H_2O)$

$\text{ Mass of excess reactant}=(0.4moles)\times (18g/mole)=7.2g$

Thus, the leftover amount of excess reagent is, 7.2 grams.

8 0

4 years ago

When lightning strikes, nitrogen molecules, n2, and oxygen molecules, o2, in the air react to form nitrates, no3, which come dow

faltersainse [42]

The reaction for what was describe in the problem is:

N₂ + 3 O₂ --> 2 NO₃

The reactants involved are nitrogen and oxygen gas. From the word itself, oxygen is an oxidizing agent. <em>Therefore, this reaction is an oxidation reaction due to the presence of the oxidizing agent.</em>

4 0

4 years ago

How many TOTAL atoms are contained in 10 molecules of TNT, C7H5N3O6?

nlexa [21]

Answer:7 atom of carbon+5atom of hydrogen +3atom of nitrogen +6 atom of oxygen =21

5 0

3 years ago

If 0.0692 mol CaCl2 is dissolved in water to make a 0.810 M solution, what is the volume of the solution?

Natali5045456 [20]

Answer:

Just ask google for help

Explanation:

I always do it and get it right

8 0

3 years ago