Answer:
S.G = 0.79.
Explanation:
Hello there!
In this case, according to the given information in the problem, it turns out possible for us to calculate the specific gravity of this alcohol by simply dividing its density, 0.79 g/mL by that of the water, 1 g/mL just as a reference for us to work with:
Thus, we plug in the densities to obtain:
Which is dimensionless as g/mL is cancelled out due to its presence on both top and bottom of the previous formula.
Regards!
The answer is C the nucleus
Answer:
See below
Step-by-step explanation:
heat gained by metal + heat lost by water = 0
m₁C₁ΔT₁ + m₂C₂ΔT₂ = 0
C₁ = -(m₂C₂ΔT₂)/(m₁ΔT₁)
The factors determining C₁ are
- mass of water
- temperature change of water (T_f - Ti)
- mass of metal
- temperature change of metal (T_f - Ti)
Any factor that makes the numerator higher or the denominator lower than what you thought, will give a calculated C₁ that is too high (and vice versa).
The major sources of uncertainty are probably in determining the temperatures, especially the initial and final temperatures of the metal. However, you will have to decide what the principal factors were in your experiment.
For example, did the metal have a chance to cool during the transfer to the calorimeter? How easy was it to determine the equilibrium temperature, etc?
Factors Affecting the Calculation of Specific Heat Capacity
<u> Too Low </u> <u> Too high </u>
Water Water
Mass less than thought Mass more than thought
Ti lower Ti higher
T_f higher T_f lower
Metal Metal
Mass more than thought Mass less than thought
Ti higher Ti lower
AgNO₃ and Cu(NO₃)₂ are dissolved in water
Answer:
Explanation:
Whenever you see molar masses in gas law questions, more often than not density will be involved. This question is no different. To solve this, however, we will first need to play with the combined ideal gas equation PV=nRT to make it work for density and molar mass. The derivation is simple but for the sake of time and space, I will skip it. Hence, just take my word for it that you will end up with the equation:M=dRTPM = molar mass (g/mol)d = density (g/L)R = Ideal Gas Constant (≈0.0821atm⋅Lmol⋅K) T = Temperature (In Kelvin) P = Pressure (atm)As an aside, note that because calculations with this equation involve molar mass, this is the only variation of the ideal gas law in which the identity of the gas plays a role in your calculations. Just something to take note of. Back to the problem: Now, looking back at what we're given, we will need to make some unit conversions to ensure everything matches the dimensions required by the equation:T=35oC+273.15= 308.15 KV=300mL⋅1000mL1L= 0.300 LP=789mmHg⋅1atm760mmHg= 1.038 atmSo, we have almost everything we need to simply plug into the equation. The last thing we need is density. How do we find density? Notice we're given the mass of the sample (0.622 g). All we need to do is divide this by volume, and we have density:d=0.622g0.300L= 2.073 g/LNow, we can plug in everything. When you punch the numbers into your calculator, however, make sure you use the stored values you got from the actual conversions, and not the rounded ones. This will help you ensure accuracy.M=dRTP=(2.073)(0.0821)(308.15)1.038= 51 g/molRounded to 2 significant figuresNow if you were asked to identify which element this is based on your calculation, your best bet would probably be Vandium (molar mass 50.94 g/mol). Hope that helped :)
