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topjm [15]
3 years ago
7

HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)

Chemistry
1 answer:
Mariulka [41]3 years ago
5 0

Answer:

Amount of H_{2}O produced will be half of its original value.

Explanation:

Balanced reaction: HCl+NaOH\rightarrow NaCl+H_{2}O

According to balanced equation, 1 mol of HCl reacts with 1 mol of NaOH to produce 1 mol of H_{2}O

If amount of reactants (NaOH and HCl) are halved then we can write-

0.5 mol of HCl reacts with 0.5 mol of NaOH to produce 0.5 mol of H_{2}O.

So, it is evident that amount of H_{2}O to be produced will be half if amount of reactants are halved.

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Answer:

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What is the definition of heat energy?
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Answer:

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If 175mL of oxygen is produced at STP, how many grams of hydrogen peroxide, H2O2
Vlad [161]

Answer:

0.53g

Explanation:

We'll begin by converting 175mL to L. This is illustrated below:

1000mL = 1L

Therefore 175mL = 175/1000 = 0.175L

Next, we shall calculate the number of mole of O2 that occupy 0.175L. This is illustrated below:

1 mole of O2 occupy 22.4L at stp.

Therefore, Xmol of O2 will occupy 0.175L i.e

Xmol of O2 = 0.175/22.4

Xmol of O2 = 7.81×10¯³ mole

Therefore, 7.81×10¯³ mole of O2 occupy 175mL.

Next, we shall determine the number of mole of H2O2 that decomposed to produce 7.81×10¯³ mole of O2. This is illustrated below:

2H2O2 —> 2H2O + O2

From the balanced equation above,

2 moles of H2O2 decomposed to produce 1 mole of O2.

Therefore, Xmol of H2O2 will decompose to produce 7.81×10¯³ mole of O2 i.e

Xmol of H2O2 = 2 x 7.81×10¯³

Xmol of H2O2 = 1.562×10¯² mole

Therefore, 1.562×10¯² mole of H2O2 decomposed in the reaction.

Finally, we shall convert 1.562×10¯² mole of H2O2 to grams. This is illustrated below:

Molar mass of H2O2 = (2x1) + (16x2) = 34g/mol

Mole of H2O2 = 1.562×10¯² mole

Mass of H2O2 =..?

Mole = mass /Molar mass

1.562×10¯² = mass /34

Cross multiply

Mass of H2O2 = 1.562×10¯² x 34

Mass of H2O2 = 0.53g

Therefore, 0.53g of Hydrogen peroxide, H2O2 were decomposition in the reaction.

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3 years ago
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can you upload a clearer photo?

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