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Juli2301 [7.4K]
3 years ago
15

Referring to an activity series, which of the following combinations of reactants would not produce a successful single-replacem

ent reaction?
Zn +CuSO4
Ca + MgSO4
Ag + SnSO4
K + Na2SO4

Chemistry
2 answers:
loris [4]3 years ago
8 0
 I believe the answer is Ca + MgSO4
bonufazy [111]3 years ago
8 0

<u>Answer:</u> The combination of reactants that will not undergo single displacement reaction is (Ag+SnSO_4)

<u>Explanation:</u>

Single-displacement reactions are defined as the reactions in which a more reactive metal displaces a less reactive metal from its chemical reaction. The reactivity of metal is judged by a series known as reactivity series.

A+BC\rightarrow AC+B

Metal A is more reactive than metal B.

The metal which is present above in the series is more reactive than the metal which is present below in the series.

For the given options:

<u>Option 1:</u>  Zn+CuSO_4

Zinc lies above in the series than copper and thus will easily replace copper from its chemical reaction.

Zn+CuSO_4\rightarrow ZnSO_4+Cu

<u>Option 2:</u>  Ca+MgSO_4

Calcium lies above in the series than magnesium and thus will easily replace magnesium from its chemical reaction.

Ca+MgSO_4\rightarrow CaSO_4+Mg

<u>Option 3:</u>  Ag+SnSO_4

Silver lies below in the series than tin and thus will not replace tin from its chemical reaction.

Ag+SnSO_4\rightarrow \text{No reaction}

<u>Option 4:</u>  K+Na_2SO_4

Potassium lies above in the series than sodium and thus will easily replace sodium from its chemical reaction.

2K+Na_2SO_4\rightarrow K_2SO_4+2Na

Hence, the combination of reactants that will not undergo single displacement reaction is (Ag+SnSO_4)

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Answer:

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Explanation:

The given equation is:

2 BaCl2+2H2SO4 \rightarrow2BaSO4+4HCl

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How many Joules are released to cool 250.0 grams of liquid water from 100°C to 0°C? The specific heat of water is 4.180 J/g.C.
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\bold{\huge{\orange{\underline{ Solution}}}}

\bold{\underline{ Given :- }}

  • <u>We </u><u>have </u><u>250g </u><u>of </u><u>liquid </u><u>water </u><u>and </u><u>it </u><u>needs </u><u>to </u><u>be </u><u>cool </u><u>at </u><u>temperature </u><u>from </u><u>1</u><u>0</u><u>0</u><u>°</u><u> </u><u>C </u><u>to </u><u>0</u><u>°</u><u> </u><u>C</u>
  • <u>Specific </u><u>heat </u><u>of </u><u>water </u><u>is </u><u>4</u><u>.</u><u>1</u><u>8</u><u>0</u><u>J</u><u>/</u><u>g</u><u>°</u><u>C</u>

\bold{\underline{ To \: Find :- }}

  • <u>We </u><u>have </u><u>to </u><u>find </u><u>the</u><u> </u><u>total</u><u> </u><u>number </u><u>of </u><u>joules </u><u>released</u><u>. </u>

\bold{\underline{ Let's \:Begin:- }}

<u>We </u><u>know </u><u>that</u><u>, </u>

Amount of heat energy = mass * specific heat * change in temperature

<u>That </u><u>is, </u>

\sf{\red{ Q = mcΔT }}

<u>Subsitute </u><u>the </u><u>required </u><u>values </u><u>in </u><u>the </u><u>above </u><u>formula </u><u>:</u><u>-</u>

\sf{ Q = 250 × 4.180 ×(0 - 100 )}

\sf{ Q = 250 × 4.180 × - 100 }

\sf{ Q = 250 × - 418}

\sf{\pink{ Q = - 104,500 J }}

Hence, 104,500 J of heat is released to cool 250 grams of liquid water from 100° C to 0° C.

\bold{\underline{ Now :- }}

<u>We </u><u>have </u><u>to </u><u>tell </u><u>whether </u><u>the </u><u>above </u><u>process </u><u>is </u><u>endothermic </u><u>or </u><u>exothermic </u><u>:</u><u>-</u>

Here, In the above process ΔT is negative and as a result of it Q is also negative that means above process is Exothermic

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Answer:

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