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ololo11 [35]
3 years ago
11

A small file or organization use a payroll program for calculating staff wages each month each employee has a unique payroll num

ber had is paid a fixed hourly rate which may be different for different employee. the system uses a master file containing long term details such as name Address, hourly,rate of pay and total pay for a year .the key field in the master file is the payroll number and the filled is stored in this field .each month by each a transaction file is produced containing details of the hours worked during that month by each employee,(a)state the type of processing used in this application and explain why this type of processing is suctable,(b) describe the processing take place each month when the payroll program is run staff with unsorted transaction file and end after the master file has been updated the pay slips have been printed,(c) explain what would happen during the processing of an employee payroll number had been entered incorrectly into the transaction file​
Chemistry
1 answer:
Rama09 [41]3 years ago
8 0

Answer:

the company is now aarav and its CEO of samruddhi and is the CEO in meeting with holika and will come in to help with holika as brainlyiest as the company's chief financial adviser to solve di problems

Explanation:

it was the most common thing that happened in my first pregnancy in my first year and I m and the other girl Bo.. were pretty good vibes for the last day of samruddhi but they are still very much a many years after I was knowing that

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Using a chemical equation to find moles of product from moles of reactant
kumpel [21]

Answer:

0.86 moles H₂O

Explanation:

To solve this problem, it is important to first determine the balanced chemical equation. The balanced equation is necessary as it will provide the mole-to-mole ratio needed to convert between moles O₂ and moles H₂O.

The unbalanced equation:

C₈H₁₈ (l) + O₂ (g) ---> CO₂ (g) + H₂O (g)

<u>Reactants:</u> 8 carbon, 18 hydrogen, 2 oxygen

<u>Products:</u> 1 carbon, 2 hydrogen, 3 oxygen

As you can see, the equation is not balanced because there are unequal amounts of each element on both sides. Balancing the equation is a matter of guessing-and-checking to see which combination of coefficients work.

The balanced equation:

2 C₈H₁₈ (l) + 25 O₂ (g) ---> 16 CO₂ (g) + 18 H₂O (g)

<u>Reactants:</u> 16 carbon, 36 hydrogen, 50 oxygen

<u>Products:</u> 16 carbon, 36 hydrogen, 50 oxygen

Now that the equation is balanced, we can use the coefficients of O₂ and H₂O to construct our mole-to-mole ratio and perform our conversion. The final answer should have 2 sig figs to match the given value (1.2 moles). The state of matter is most likely not necessary to include in your final answer.

1.2 moles O₂          18 moles H₂O
---------------------  x  -----------------------  =  0.86 moles H₂O
                                25 moles O₂

3 0
2 years ago
H2(g) + F2(g)2HF(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.20 moles
abruzzese [7]

<u>Answer:</u> The value of \Delta S^o for the surrounding when given amount of hydrogen gas is reacted is -31.02 J/K

<u>Explanation:</u>

Entropy change is defined as the difference in entropy of all the product and the reactants each multiplied with their respective number of moles.

The equation used to calculate entropy change is of a reaction is:

\Delta S^o_{rxn}=\sum [n\times \Delta S^o_{(product)}]-\sum [n\times \Delta S^o_{(reactant)}]

For the given chemical reaction:

H_2(g)+F_2(g)\rightarrow 2HF(g)

The equation for the entropy change of the above reaction is:

\Delta S^o_{rxn}=[(2\times \Delta S^o_{(HF(g))})]-[(1\times \Delta S^o_{(H_2(g))})+(1\times \Delta S^o_{(F_2(g))})]

We are given:

\Delta S^o_{(HF(g))}=173.78J/K.mol\\\Delta S^o_{(H_2)}=130.68J/K.mol\\\Delta S^o_{(F_2)}=202.78J/K.mol

Putting values in above equation, we get:

\Delta S^o_{rxn}=[(2\times (173.78))]-[(1\times (130.68))+(1\times (202.78))]\\\\\Delta S^o_{rxn}=14.1J/K

Entropy change of the surrounding = - (Entropy change of the system) = -(14.1) J/K = -14.1 J/K

We are given:

Moles of hydrogen gas reacted = 2.20 moles

By Stoichiometry of the reaction:

When 1 mole of hydrogen gas is reacted, the entropy change of the surrounding will be -14.1 J/K

So, when 2.20 moles of hydrogen gas is reacted, the entropy change of the surrounding will be = \frac{-14.1}{1}\times 2.20=-31.02J/K

Hence, the value of \Delta S^o for the surrounding when given amount of hydrogen gas is reacted is -31.02 J/K

7 0
3 years ago
What did the experiments of scientists after John Dalton reveal about his
EastWind [94]

A. Dalton's theory that atoms could not be divided was incorrect

3 0
3 years ago
N2+3H2---&gt; 2NH3
irakobra [83]
Hello!

A) H<span>ow many grams of hydrogen are necessary to react completely with 50.0g of nitrogen in the above reaction?

The balanced chemical reaction is the following one:

N</span>₂(g) + 3H₂(g) → 2NH₃(g)

To calculate the amount of hydrogen necessary we will use the following conversion factor to go from grams of nitrogen to grams of hydrogen:

50 gN_2* \frac{1 mol N_2}{28,013 g N_2}* \frac{3 moles H_2}{1 mol N_2}* \frac{2,016 g H_2}{1 mol H_2}=10,7950 g H_2

So, 10,7950 grams of H₂ are required to react with 50 g of nitrogen

<span>B) How many grams of ammonia are produced in the reaction from the previous problem?

</span>The balanced chemical reaction again is the following one:

N₂ + 3H₂ → 2NH₃

To calculate the amount of ammonia produced we will use the following conversion factor to go from grams of nitrogen to grams of ammonia:

50 gN_2* \frac{1 mol N_2}{28,013 g N_2}* \frac{2 moles NH_3}{1 mol N_2}* \frac{17,031 g NH_3}{1 mol NH_3}=60,7968 g NH_3

So, 60,7968 grams of NH₃ are produced from 50 g of nitrogen

C) <span>How many grams of silver chloride are produced from 5.0g of silver nitrate reacting with an excess of barium chloride?

The balanced chemical equation for the reaction is the following one:

2AgNO</span>₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂

To calculate the mass of Silver Chloride produced we will use the following conversion factor to go from grams of Silver Nitrate to grams of Silver Chloride:

5 g AgNO_3* \frac{1 mol AgNO_3}{169,87 g AgNO_3}* \frac{2 moles AgCl}{2 moles AgNO_3}* \frac{143,32 g AgCl}{1 mol AgCl}=4,2185 g AgCl

So, 4,219 g of AgCl are produced from the reaction of 5 g of AgNO₃ 

D) <span>How much barium chloride is necessary to react with the silver nitrate in the previous problem?

</span>The balanced chemical equation for the reaction is the following one:

2AgNO₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂

To calculate the mass of Barium Chloride necessary we will use the following conversion factor to go from grams of Silver Nitrate to grams of Barium Chloride:

5 g AgNO_3* \frac{1 mol AgNO_3}{169,87 g AgNO_3}* \frac{1 mol BaCl_2}{2 moles AgNO_3}* \frac{208,23 g BaCl_2}{1 mol BaCl_2}=3,08 g BaCl_2


So, 3,08 g of BaCl₂ are produced from the reaction of 5 g of AgNO₃ 

Have a nice day!
4 0
3 years ago
Write a balanced chemical equation for the reaction of gaseous nitrogen dioxide with hydrogen gas to form gaseous ammonia and li
LenKa [72]
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3 0
3 years ago
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