Calculate the following to the correct number of signifi- cant figures. Assume that all these numbers are measurements. (a) x5 17.2 1 65.18 2 2.4
(b) x5 13.0217 17.10
(c) x5 (0.0061020)(2.0092)(1200.00)

See below

Explanation:

First, you need to know what a significant figure means.

The significant figures in a measurement consist of all the certain digits in one measurement, including one uncertain or estimated digit.

With that being said, the second thing we need to do is to correct the exercise. According to an external source, the exercise is the following:

a) x = 17.2 + 65.18 - 2.4

In this case, we can say that 17.2 and 2.4 has the uncertain digit at the end, but in 65.18 it's the 8. Therefore, when we make the sum of all of this we have:

x = 17.2 + 65.18 - 2.4 = 79.98

The last digit is the uncertain digit, therefore, we won't include this digit. So the final result would have 3 significant figure. However 8 surpass 5, and hence, we should approximate our result. Then our final result is:

x = 80.0

b) x = 13.0217 / 17.10

The last digit of the 13, is the uncertain. So, doing this:

x = 13.0217 / 17.10 = 0.761502924

With the correct significant figure, this would be only 4 so:

x = 0.7615

c) x = (0.0061020)*(2.0092)*(1200.00)

Applying the same principle as before:

x = (0.0061020)*(2.0092)*(1200.00) = 14.712

Hope it helps

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: